Mercury(II) bromide

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Mercury(II) bromide
IUPAC name Mercury(II) bromide
Other names Mercuric bromide
Identifiers
CAS number [7789-47-1]
RTECS number OV7415000
Properties
Molecular formula HgBr2
Molar mass 360.41 g/mol
Appearance white solid
Density 6.03 g/cm³, solid
Melting point

236 °C
Boiling point

322 °C
Solubility in water  ?
Hazards
EU classification Very toxic (T+)
Dangerous for
the environment (N)
R-phrases R26/27/28, R33, R50/53
S-phrases S13, S28, S45, S60, S61[1]
Flash point non-flammable
Related compounds
Other anions Mercury(II) fluoride
Mercury(II) chloride
Mercury(II) iodide
Other cations Zinc bromide
Cadmium bromide
Mercury(I) bromide
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references

Mercury(II) bromide or mercuric bromide is the chemical compound composed of mercury and bromine with the formula HgBr2. This white crystalline solid is a laboratory reagent. Like mercury(II) chloride, it is extremely toxic.

[edit] Reactions

Mercury(II) bromide is used as a reagent in the Koenigs–Knorr reaction, which forms glycoside linkages on carbohydrates [2] [3].


It is also used to test for the presence of arsenic, as recommended by the Pharmacopoeia [4]. The arsenic in the sample is first converted to arsine gas by treatment with hydrogen. Arsine reacts with mercury(II) bromide:[5]

AsH3 + HgBr2 → As(HgBr3) + HBr

The white mercury(II) bromide will turn yellow, brown, or black if arsenic is present in the sample [6].

Mercury(II) bromide reacts violently with elemental indium at high temperatures [7] and, when exposed to potassium, can form shock-sensitive explosive mixtures [8].

[edit] References

  1. ^ 437859 Mercury(II) bromide 99.998%. Sigma-Aldrich. Retrieved on 2008-05-29.
  2. ^ Horton, Derek, Advances in Carbohydrate Chemistry and Biochemistry, Amsterdam: Elseveir Academic Press, pp. 76, ISBN 0120072599, <http://books.google.com/books?id=E22gW9CbU_0C&pg=PA76&dq=%22mercury(II)+bromide%22&as_brr=3&sig=0vbTilhQ61APnPcw07PlFt-eEDw#PPA76,M1>. Retrieved on 2007-05-29 
  3. ^ Stick, Robert V., Carbohydrates: The Sweet Molecules of Life, San Diego: Academic Press, pp. 125, ISBN 0126709602, <http://books.google.com/books?id=-MtjsUMB6ogC&pg=PA125&dq=%22mercury(II)+bromide%22&lr=&as_brr=3&sig=PjRI5fbHysGXw_DHbhRzEeqNE84#PPA125,M1>. Retrieved on 2007-05-29 
  4. ^ Pederson, Ole, Pharmaceutical Chemical Analysis, Boca Raton, FL: CRC Press, pp. 107, ISBN 0849319781, <http://books.google.com/books?id=R7ZxXS5DZj8C&pg=PT125&dq=%22mercury(II)+bromide%22&lr=&as_brr=3&sig=XrgXrUopvgaFD3jWqvVx88KbgC8#PPT125,M1>. Retrieved on 2007-05-29 
  5. ^ Odegaard, Nancy & Sadongei, Alyce, Old Poisons, New Problems, Rowman Altamira, pp. 58, ISBN 0759105154, <http://books.google.com/books?id=QLU0SVlruCMC&pg=PA58&dq=%22mercury(II)+bromide%22&lr=&as_brr=3&sig=biYpKuAxjpGhj1lpGniTM6jiFv0>. Retrieved on 2007-05-29 
  6. ^ Townsend, Timothy G. & Solo-Gabriele, Helena, Environmental Impacts of Treated Wood, Boca Raton, FL: CRC Press, pp. 339, ISBN 0849364957, <http://books.google.com/books?id=ENJL1UMdGTUC&pg=PT361&dq=%22mercury(II)+bromide%22&lr=&as_brr=3&sig=fGTI_exu0D4eA7I-c7nLwKYfUqQ>. Retrieved on 2007-05-29 
  7. ^ Bretherick, L.; Urben, P. G. & Pitt, Martin John, Bretherick's Handbook of Reactive Chemical Hazards, Elseveir Academic Press, pp. 110, ISBN 075063605X, <http://books.google.com/books?id=UOxbX8q6DXsC&pg=PA1726&dq=%22mercury(II)+bromide%22&as_brr=3&sig=Db6GjtyYywXRtmeQFjbeLSco374#PPA110,M1>. Retrieved on 2007-05-29 
  8. ^ Bretherick, L.; Urben, P. G. & Pitt, Martin John, Bretherick's Handbook of Reactive Chemical Hazards, Elseveir Academic Press, pp. 1276, ISBN 075063605X, <http://books.google.com/books?id=UOxbX8q6DXsC&pg=PA1726&dq=%22mercury(II)+bromide%22&as_brr=3&sig=Db6GjtyYywXRtmeQFjbeLSco374#PPA110,M1>. Retrieved on 2007-05-29 
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